Presentation on theme: "Thinking (Electro) Negatively Making Sense page 139."— Presentation transcript:
Thinking (Electro) Negatively Making Sense page 139
Electronegativity values increase from left to right on a period and up a group.
Electronegativity Difference The difference of electronegativity values (EV) of two atoms determines the type of bond is between them. Type of bondEV difference Nonpolar bond0 to 0. 3 Polar bond0.4 to 1.7 Ionic Bond 1.8 to 3.3
3 Types of Bonds 1.Bonded electrons are equally shared in a nonpolar covalent bond. It consists of nonmetals and there is no charge. Electronegativity difference is between 0 to 0.3. Ex: Cl - Cl
2. A polar covalent bond consists of bonded electrons that are shared unequally between nonmetals. The electronegativity value difference is between 0.4 to 1.7 which results in partial charges. Ex: H EV =2.10 Cl EV =3.163.16-2.10 = 1.06 * Bonded electrons are pulled toward the chlorine atom.
3. An ionic bond is when a nonmetal atom gains an electron(s) from a metal atom. The electronegativity value difference is between 1.8 to 3.3. The metal atom becomes a positive ion (caiton) and the nonmetal atom becomes a negative ion (anion). Ex: Na EV = 0.93Cl EV = 3.163.16-0.93= 2.23 Na + Cl -
Note: CCl 4 is a nonpolar molecule even though C-Cl is polar bond. Remember CCl 4 is symmetrical.
Exercises page. 139 What is the electronegativity value difference and type of bond for the following? 1.C-S 2.Li-F 3.H-I 4.C-O
Exercises page. 141 What is the electronegativity value difference and type of bond for the following? 1.C-S2.55-2.58=0.03, nonpolar bond 2.Li-F0.98-3.98=3.00, ionic bond 3.H-I2.10-2.66=0.56, polar bond 4.C-O2.55-3.44=0.89, polar bond